Why is $LiF$ almost insoluble in water whereas $LiCl$ is soluble not only in water but also in acetone?

(N/A) $LiF$ is almost insoluble in water due to its very high lattice energy. The fluoride ion $(F^-)$ is very small,leading to a strong electrostatic attraction with the $Li^+$ ion,resulting in a high lattice energy that is not compensated by the hydration energy.
In contrast,$LiCl$ has a lower lattice energy because the chloride ion $(Cl^-)$ is larger. Additionally,$LiCl$ possesses significant covalent character due to the polarizing power of the small $Li^+$ ion (Fajans' rule),which makes it soluble in organic solvents like acetone.
Therefore,the solubility of $LiCl$ in water is driven by favorable hydration energy,while its solubility in acetone is attributed to its covalent nature.